🤓 Based on our data, we think this question is relevant for Professor Boehr's class at PSU.

We’re being asked to **calculate the lattice energy** of **rubidium chloride (RbCl)**.

Recall that ** lattice energy** is the energy required to combine two gaseous ions into a solid ionic compound:

M^{x+}(g) + N^{y–}(g) → M_{y}N_{x}(s)

To calculate for lattice energy, we need to do the ** Born-Haber cycle for RbCl**.

We start with the corresponding formation equation for RbCl:

Rb(s) + 1/2 Cl_{2}(g) → RbCl(s), **ΔH˚ _{f}**

The enthalpy of formation (ΔHf) of rubidium chloride is -430.5 kJ/mol. The enthalpy of sublimation for rubidium is 86 kJ/mol, and the first ionization energy of rubidium is 402 kJ/mol. The bond dissociation energy of (g) is 243 kJ/mol, and the electron affinity of chlorine is -349 kJ/mol. Calculate the lattice energy of RbCl (s), in kJ/mol.

a. -170

b. -691

c. +260.5

d. -812..5

e. -260.5